chemistry

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How much heat in kilojoules is evolved in converting 1.00 mol of steam at 145 Celsius to ice at -50 Celsius?
Please, all particular steps and conversions between mole and grams of steam, H2O and ice. Thanks!

  • chemistry -

    q1 = heat evolved in moving steam from 145 to 100.
    q1 = mass steam x specific heat steam x (Tfinal-Tinital) where Tfinal is 100 and Tinitial is 145.

    q2 = heat evolved when steam at 100 C condenses to liquid at 100 C.
    q2 = mass x heat vaporization

    q3 = heat evolved in moving water from 100 C to zero.
    q3 = mass water x specific heat water x (Tfinal-Tinitial) where T final is zero and Tinitial is 100.

    q4 = heat evolved on freezing water at zero to ice at zero.
    q4 = mass water x heat fusion.

    q5 = heat evolved in moving ice from zero to -50.
    q5 = mass ice x specific heat ice x (Tfinal-Tinitial) where Tfinal is -50 and Tinitial is zero.

    Total Q = q1+q2+q3+q4+q5

  • chemistry -

    57.8kJ

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